Redox reaction
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abo
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Redox reaction


Can somebody out here help me with this redox reaction? it says that KMnO4 reacts with K2C2O4 in acidic conditions and the products are MnO2 and CO2?

this is how I did it:

[KMnO4 + (4H+) + (3e-) -----> MnO2 + (K+) + 2H2O] *2

[K2C2O4 ------> 2CO2 + (2K+) + (2e-) ] *3
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2KMnO4 + 3K2C2O4 + (8H+) ------> 2MnO2 + 6CO2 + (8K+) + 4H2O


Last edited by abo on Tue Apr 02, 2019 3:38 am; edited 1 time in total
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ChenBeier
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From the writing and calculation its ok. But in practise in acidic conditions Permanganate will be reduced to Mn2+. Manganese dioxide you get at neutral or alkaline conditions.
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abo
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Thank you very much for your answer. As I said the products were given in the question so I had to follow the instructions.
Anyways I have got a balanced equation and based on that I tried to calculate the mass of CO2.

I would be grateful if you could have a look at my solution Smile.
OBS! I used the dotted line so that every value comes under the respective chemical formula.

......2KMnO4 + 3K2C2O4 + (8H+) ------> 2MnO2 + 6CO2 + (8K+) + 4H2O
......2 mole......3 mole ............................................6 mole

.......2*158 g.....3*166 g...........................................6*44 g

given: 22 g......7 g.................................................. x g

the limiting substance is K2C2O4 and therefore i will use it to do my calculation: x = (6*44*7) / 3*166) ≈ 3.71 g

Now (measured in gram) how much methane you will get if you react the amount of CO2 you have got with H2?
CO2 + 4H2 ------> CH4 + 2H2O
1 mole....................1 mole

44 g......................16 g

3,71 g...................... s g
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s= (16*3,71)/44 ≈ 1,35g
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ChenBeier
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Sounds good for me.
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abo
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thank you so much for taking the time to look at it! Smile
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